Question
The rate constant of reaction is 1.5 10^7\ s ^ -1 at 300 K and 3.0 10^7\ s ^ -1 at 330 K. What is the activation energy for the reaction? [ R 2.303 = 19.15\ JK ^ -1 mol ^ -1 ]
MHT CET
Chemistry
Chemical Kinetics
2026
MHT CET 2026 (16 April Shift 1)
MHT CET Chemistry Question (2026) — Solution
Options
- A. 18.02\ kJ mol ^ -1
- B. 20.1\ kJ mol ^ -1
- C. 19.02\ kJ mol ^ -1
- D. 21.5\ kJ mol ^ -1
Answer
C. 19.02\ kJ mol ^ -1
Step-by-step solution
Using the Arrhenius equation: ( k_2 k_1 ) = E_a 2.303 R ( T_2 - T_1 T_1 T_2 ) Substituting the given values: ( 3.0 10^7 1.5 10^7 ) = E_a 19.15 ( 330 - 300 300 330 ) (2) = E_a 19.15 ( 30 99000 ) 0.301 = E_a 19.15 ( 1 3300 ) E_a = 0.301 19.15 3300 E_a = 19021.695\ J mol ^ -1 E_a 19.02\ kJ mol ^ -1 Answer: 19.02\ kJ mol ^ -1
Related: Chemistry — Chemical Kinetics · All PYQ Banks